
Which of the following species has the highest bond energy?
(A)-
(B)-
(C)-
(D)-
Answer
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Hint: Bond energy is the energy required to break one mole of a bond to separate the bonded atoms in the gaseous state. It can also be defined as the amount of energy released when one mole of a particular bond is formed between gaseous atoms. Bond energy of a bond is directly proportional to the multiplicity of the bond, i.e. its bond order.
Complete step by step answer:
Bond order tells us the number of covalent bonds present in a molecule. We know that bond energy increases with the bond order. So the molecule having the highest bond order will have the highest bond energy.
Thus, let us calculate the bond order in the given species.
Bond order is mathematically calculated as half the difference between the number of electrons in the bonding and number of electrons in the antibonding orbitals. If and are the number of bonding and antibonding electrons, respectively, then bond order is given as
Electronic configuration of oxygen, O (Z=8): .
Electronic configuration of oxygen molecule, :
Bond order of peroxide ion
Oxygen molecule ( ) has 16 electrons. It gains 2 electrons to form ion. The two electrons gained will be added into half filled and such that the electronic configuration of is .
Now, the total number of electrons in bonding molecular orbitals, = 10
Total number of electrons in the antibonding molecular orbitals, = 8
Therefore, the bond order of will be
Bond order =
Bond order =
Bond order of ion.
One electron is lost from (or ) molecular orbital of molecule to form ion. Since, one electron is lost from antibonding molecular orbital, the electronic configuration of ion becomes
.
Total number of electrons in bonding molecular orbitals, = 10
Number of electrons in the antibonding molecular orbitals, = 5
Therefore, bond order =
Bond order of superoxide ion
molecule gains one electron into (or ) to form ion. Now the electronic configuration of is .
Number of bonding electrons, = 10
Number of antibonding electrons, = 7
Therefore, bond order of =
Bond order of oxygen molecule,
We know that electronic configuration of molecule is given as
molecule has 10 electrons in bonding molecular orbitals and 6 electrons in antibonding molecular orbitals, thus its bond is calculated to be
Therefore, the bond order of the given species follows the order, i.e. .
Since, bond energy increases with the increase of bond order. So, the bond energy of the species also follows the same order as the bond order, i.e.
Thus, has the highest bond order, and hence the highest bond energy.
So, the correct answer is “Option B”.
Note: Greater the bond order, higher the bond energy and hence, greater is the stability. Note that the energy of is less than that of and molecular orbitals and energy of both the -orbitals, and is the same in case of , i.e. .
Complete step by step answer:
Bond order tells us the number of covalent bonds present in a molecule. We know that bond energy increases with the bond order. So the molecule having the highest bond order will have the highest bond energy.
Thus, let us calculate the bond order in the given species.
Bond order is mathematically calculated as half the difference between the number of electrons in the bonding and number of electrons in the antibonding orbitals. If
Electronic configuration of oxygen, O (Z=8):
Electronic configuration of oxygen molecule,
Bond order of peroxide ion
Oxygen molecule (
Now, the total number of electrons in bonding molecular orbitals,
Total number of electrons in the antibonding molecular orbitals,
Therefore, the bond order of
Bond order =
Bond order =
Bond order of
One electron is lost from
Total number of electrons in bonding molecular orbitals,
Number of electrons in the antibonding molecular orbitals,
Therefore, bond order =
Bond order of
Number of bonding electrons,
Number of antibonding electrons,
Therefore, bond order of
Bond order of oxygen molecule,
We know that electronic configuration of
Therefore, the bond order of the given species follows the order, i.e.
Since, bond energy increases with the increase of bond order. So, the bond energy of the species also follows the same order as the bond order, i.e.
Thus,
So, the correct answer is “Option B”.
Note: Greater the bond order, higher the bond energy and hence, greater is the stability. Note that the energy of
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